* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download g - Porterville College Home
Molecular orbital diagram wikipedia , lookup
Coordination complex wikipedia , lookup
Computational chemistry wikipedia , lookup
Radical (chemistry) wikipedia , lookup
Atomic orbital wikipedia , lookup
Lewis acid catalysis wikipedia , lookup
Nanofluidic circuitry wikipedia , lookup
Cation–pi interaction wikipedia , lookup
Electrolysis of water wikipedia , lookup
Electronegativity wikipedia , lookup
Resonance (chemistry) wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
Stoichiometry wikipedia , lookup
Debye–Hückel equation wikipedia , lookup
Chemistry: A Volatile History wikipedia , lookup
Electrochemistry wikipedia , lookup
Bond valence method wikipedia , lookup
Metallic bonding wikipedia , lookup
Hypervalent molecule wikipedia , lookup
Inorganic chemistry wikipedia , lookup
Rutherford backscattering spectrometry wikipedia , lookup
Acid dissociation constant wikipedia , lookup
Biochemistry wikipedia , lookup
Nucleophilic acyl substitution wikipedia , lookup
Molecular dynamics wikipedia , lookup
History of chemistry wikipedia , lookup
Electron configuration wikipedia , lookup
Hydrogen atom wikipedia , lookup
Chemical bond wikipedia , lookup
Homoaromaticity wikipedia , lookup
Acid–base reaction wikipedia , lookup
Metalloprotein wikipedia , lookup
History of molecular theory wikipedia , lookup
Atomic theory wikipedia , lookup
IUPAC nomenclature of inorganic chemistry 2005 wikipedia , lookup
Chemistry 106 Expectations As the title indicates, these are what I would expect of you, when you come into the classroom. These should be common sense, but I am reiterating them for students. I also provide what you can expect of me. Buzz Piersol Daily Classroom Expectations of Students Regularly attend class Arrive to class on time Read and understand the syllabus and policies within Be aware of campus policies and be familiar with the PC catalog Cell phone is off or set on vibrate/silent Bring all materials to every class meeting: pencil, notebook, calculator, textbook Do not bring or eat food/drink to class (water OK) Retain all handouts throughout the semester Read the textbook Perform homework/lab assignments on time Prepare for quizzes/mid-term/final exam Contact instructor outside of class, if making below-than-average progress Be prepared to learn and participate Daily Laboratory Expectations of Students Arrive to lab on time Turn cell phone off or set it to vibrate/silent Bring/Borrow and wear safety goggles during experiments Wear closed-toe shoes (i.e. not sandals) Do not wear loose/dangling jewelry or loose clothing Tie-back long hair. Read the procedure and follow instructions for daily experiment Notify instructor of any accident/spill/fire (including glass breakage) Do not eat/drink in the laboratory Be prepared to learn and participate What Students Can Expect of the Instructor Arrive to class/lab on time Frequently invite questions, and answer all questions Communicate with students respectfully Be prepared for daily activity/lecture/laboratory with all supporting/necessary materials. Return laboratory assignments in a reasonable amount of time. Return exams in a reasonable amount of time. Regularly notify students of progress Assign grades fairly, according to the syllabus, and high academic standards Encourage student learning CHEM 106 Summer 2016 Online Homework – Sapling Learning Philosophy Your online homework was selected and tailored with student learning in mind. Often, students do their homework at home or away from the college, so they do not have access to the professor. When they have trouble, they can either contact the professor by email or wait until the next class meeting. Online homework allows immediate feedback and encourages online contact with the instructor. Sapling Learning was selected for online homework for many reasons. They specialize in chemistry homework. The assignments also provide hints and assistance in a stepwise fashion—this makes learning with homework a better experience. Purchase You can purchase the online homework in one of two ways. You can purchase a physical package in the bookstore or online when you register. Registration When you register with sapling, you can use your email address or a Facebook account (details below). If you choose email, it is recommended that you use your Porterville College email account. Be sure to enter your email address correctly when you register—this is a very important step! The PC email typically has a pattern “your.name####@email.portervillecollege.edu”. It is easy to mistype at least one character incorrectly. See below for registration. 1. Go to https://www.saplinglearning.com/ibiscms 2. If you already have a Sapling Learning account, log in then skip to step 4, otherwise, click CREATE AN ACCOUNT. 3, If you have Facebook account, you can use it to quickly create a Sapling Learning account, otherwise, fill in the fields and register a new account. 4. Find your course in the list (you may need to expand the subject and term categories) and click the link. 5. Use the bookstore package to register for the online homework or select a payment option and follow the remaining instructions. Once you have registered and enrolled, you can log in at any time with any computer on the internet to review and complete or your homework assignments. During sign up - and throughout the term - if you have any technical problems or grading issues, send an email to [email protected] explaining the issue. The Sapling support team should be able to help with support issues. If you have homework questions, email Buzz at [email protected] or text at 559-791-8346. CHEM 106 Homework Assignments (mostly online) Week Assignment Available Date Due Date 1 Practice Assignment Wednesday, June 01 Wednesday, June 15 1 Math Review Wednesday, June 01 Wednesday, June 15 1 HW1&2 Wednesday, June 01 Wednesday, June 15 1 HW2&3 Wednesday, June 01 Wednesday, June 15 2 HW4 Monday, June 06 Monday, June 20 2 HW11 Wednesday, June 08 Wednesday, June 22 3 Practice Drawing Molecules Wednesday, June 08 -- 3 HW12 Monday, June 13 Monday, June 27 3 HW5 Wednesday, June 15 Wednesday, June 29 4 HW6&7 Monday, June 20 Tuesday, July 5 * 4 HW8 Wednesday, June 22 Wednesday, July 6 5 HW9 Monday, June 27 Monday, July 11 5 HW13 Wednesday, June 29 Wednesday, July 13 6 HW14 Monday, July 4 Monday, July 18 6 HW15 Wednesday, July 6 Wednesday, July 20 * HW6&7 assignment due on July 5 as July 4 is a holiday (Independence Day) 6/6/2016 Conversion Factors NOTE: All equalities are EXACT (i.e. ∞ number of SF), except those marked with an asterisk (*) ENGLISH/US SYSTEM Be familiar with each unit, abbreviation and equality below. Mass Length Volume 1 ton = 2000 lb (pounds) 1 lb = 16 oz (ounces) 1 mi (mile) = 5,280 ft (feet) 1 yd (yard) = 3 ft 1 ft = 12 in (inch) 1 gal (gallon) = 4 qt (quart) 1 qt = 2 pt (pint) 1 pint = 2 cups 1 qt = 32 fl oz (fluid ounces) COMMON METRIC SYSTEM BASE UNITS SI SYSTEM UNITS Length: Mass: Volume: Length: Mass: Time: Temperature: meter (m) gram (g) liter (L) meter (m) kilogram (kg) second (s) kelvin (K) Any unit can be modified by by adding a prefix to a base unit. The value of the prefixed unit is the numerical equivalent of the base unit (e.g. 1 µL = .000001 L) PREFIX mega kilo deci centi milli micro nano ABBR M k d c m µ n NUMERICAL EQUIVALENT 106 or 1,000,000 103 or 1,000 100 or 1 10-1 or .1 10-2 or .01 10-3 or .001 10-6 or .000,001 10-9 or .000,000,001 TEMPERATURE CONVERSIONS: TF = 1.8TC + 32 TC = TF − 32 1.8 TK = TC + 273 TC = TK − 273 OTHER IMPORTANT METRIC EQUALITIES: 1 cubic centimeter (cm3) = 1 mL 1 angstrom (Ǻ) = 10-10m ENGLISH - METRIC BRIDGE EXAMPLES Mass 1 lb = 453.6 g * 1 kg = 2.205 lb * Length 1 in = 2.54 cm 1 m = 1.094 yd * 1 mi = 1.609 km * Volume 1 L = 1.0567 qt* 3 1 ft = 28.32 L * Drawing Simple Lewis Structures 1. Count valence electrons contributed from all atoms. a. For anions, add one electron for each negative charge. b. For cations, subtract one electron for each charge. Use this number of electrons exactly for bonding and non-bonding in the structure. These electrons must be distributed to all atoms such that each has an octet except hydrogen (“duet”). 2. Place atoms around a central atom (lone atom, or the atom with the lowest Electronegativity). 3. Place one bond (2 electrons) between each outer atom and the central atom. Subtract from the original electron count. 4. Place lone pairs (2 unshared electrons—non-bonding electron pairs) on the outer atoms (except H), until each has satisfied the octet or until there are no more remaining. Subtract from the count as you use them. 5. If there are remaining electrons, place them on the central atom, in pairs. Subtract electrons used. 6. If the central atom does not meet the octet, then share previously assigned nonbonding electrons from outer atoms to form double and triple bonds. Valence Shell Electron Pair Repulsion Theory Groups 0 Lone Pairs 1 Lone Pair 2 Lone Pairs 180° 2 Linear 120° 3 <120° Trigonal Planar Bent 109.5° 4 <109.5° Tetrahedral Trigonal Pyramid Note: any structure with just two atoms bonded is linear <109.5° Bent NOMENCLATURE CHART OXYACIDS AND THEIR ANIONS Acids (name of compound) Anions (form latter part of name of ionic compound) HNO3 NO3− nitrate − nitrite nitric acid HNO2 nitrous acid NO2 HClO4 perchloric acid ClO4− perchlorate − chlorate HClO3 chloric acid ClO3 HClO2 chlorous acid ClO2− chlorite HClO hypochlorous acid ClO− hypochlorite HC2H3O2 acetic acid acetate H2CO3 carbonic acid C2H3O2− HCO3− H2SO4 sulfuric acid HSO4− H2SO3 sulfurous acid HSO3− H3PO4 phosphoric acid Each of these 4 ions and 4 acids form similar structures and names for Br, and I instead of Cl. hydrogen carbonate or bicarbonate CO32− carbonate hydrogen sulfate or bisulfate hydrogen sulfite or bisulfite SO42− sulfate SO32− sulfite H2PO4- dihydrogen phosphate HPO42− hydrogen phosphate PO43− phosphate BINARY & OTHER NON-OXYACIDS AND THEIR ANIONS HF(aq) hydrofluoric acid F− fluoride HCl(aq) hydrochloric acid Cl− chloride HBr(aq) hydrobromic acid Br− bromide HI(aq) hydroiodic acid I− iodide H2S(aq) hydrosulfuric acid S2− sulfide HCN(aq) hydrocyanic acid CN− cyanide MISCELLANEOUS IONS H− OH− MnO4 − CrO42− Cr2O7 2− O22− AsO4 GREEK PREFIXES (BINARY MOLECULAR CPDS) hydride NH4 hydroxide + ammonium 1 mono- 6 hexa- Ag+ silver 2 di- 7 hepta- permanganate Zn2+ zinc 3 tri- 8 octa- chromate Cd2+ cadmium 4 tetra- 9 nona- dichromate Al3+ aluminum 5 penta- 10 deca- peroxide 3− arsenate it's the only non-metal cation we will see! VARIABLE VALENCE (CHARGE) METAL IONS Ion stock name traditional name (for information only) Cu1+ copper(I) cuprous Cu2+ copper(II) cupric mercury(I) mercurous Hg2+ mercury(II) mercuric Au1+ gold(I) aurous Au3+ gold(III) auric Cr2+ chromium(II) chromous Cr3+ chromium(III) chromic Mn2+ manganese(II) manganous Mn3+ manganese(III) manganic Fe2+ iron(II) ferrous Fe3+ iron(III) ferric Co2+ cobalt(II) cobaltous Co3+ cobalt(III) cobaltic Ni2+ nickel(II) nickelous Ni3+ nickel(III) nickelic Sn2+ tin(II) stannous Sn4+ tin(IV) stannic Pb2+ lead(II) plumbous Pb4+ lead(IV) plumbic Hg2 2+ (Note: This is the only metal polyatomic ion!) Anions end in -ide Cation name is same as element 1A COMMON IONS BASED ON PERIODICITY 3A 4A 2A 5A 6A 7A H + Li Na + N 2+ 3+ Mg Al 3B K + Rb + + Cs Ca Sr 2+ 4B 5B 6B 7B 8B 1B 2B Cr2+ Cr3+ Mn2+ Mn3+ Fe2+ Fe3+ Co2+ Co3+ Ni2+ Ni3+ Cu+ Cu2+ Zn2+ Ga3+ P 3- O 2- 2- S - F - Cl Br 2+ Ag+ Cd2+ In3+ Sn2+ Sn4+ 2+ Au+ Hg22+ Au3+ Hg2+ Pb2+ Pb4+ Ba 3- - I - - 8A Inorganic Nomenclature Guidelines First determine whether you compound is an ionic compound, an acid, or binary molecular. Ionic Compound – starts with a metal or ammonium (NH4+). Go to procedure 1. Acid – Starts with H (except H2O and H2O2). Go to procedure 2. Binary Molecular – Two non-metal elements. Go to procedure 3. 1. Ionic Compound: Name is “cation anion”. Determine the names each of the cation and anion. Divide the formula into the cation and anion. Use the formulas to determine the names of each. a. Name cation. Simple metal, variable valence or NH4+? i. Simple metal: Cation is the name of the element. ii. Variable valence: Determine the charge of the metal by looking at the charge of the anion and the formula subscripts. Roman numeral name of cation will be element (charge) where charge is a roman numeral (without plus sign!). Classical name ends in “– ous” if lower charged metal and “–ic” if higher charged. iii. NH4+ cation name is ammonium. b. Name anion. Is the anion a Non-metal or polyatomic anion? i. Non-metal anion: Anion name is name of the element with “–ide” ending. ii. Polyatomic ion: Oxyanion or other? 1. Oxyanion: Name derived from the name of the non-metal that oxygen is paired with. Larger subscript of oxygen in a series name ends in “–ate.” Smaller subscript of oxygen in a series name ends in “–ite.” See Oxyanion tips. 2. Other: Some other polyatomic anions include CNcyanide, OH- hydroxide, peroxide O222. Acid: Last word of acid name is always “acid.” Determine whether the acid has oxygen or not: a. Oxyacid: Name derived from non-metal that accompanies the oxyanion i. “–ate” oxyanion becomes “-ic acid” (higher number of oxygens) ii. “–ite” oxyanion becomes “-ous acid” (lower number of oxygens) b. Non-Oxyacid: Name starts with “hydro-“ and the rest of the name is derived from anion: “-ide” becomes “hydro[anion]-ic acid” 3. Binary Molecular: Two non-metals. Name is composed of two words: a. First word is the first element in the formula. Second word is the second element with the usual modified “-ide” ending. b. Prefixes are added to each word based on the subscript of each element. Refer to Greek prefix table (e.g. tri = 3 atoms) c. Prefix exception: Mono is never used on the first word regardless if there is one atom of that element. (e.g. carbon monoxide not monocarbon monoxide) d. Prefix vowel omitted if similar vowel sounds run together by addition of the prefix. (e.g. carbon monoxide NOT carbon monooxide) Notes: Be aware of the following compounds, which use a common name. Common names do not follow systematic (IUPAC) procedure: H2O water H2O2 hydrogen peroxide NH3 ammonia CH4 methane Oxyanion Tips: • • • • • • • • Oxyanion names will always end in –ate or –ite. Since oxyanions are anions (negatively charged ions), they will always be found paired with a cation and form the latter part of a name and formula. Do not confuse the naming of oxyanions (end in –ate or –ite) with the naming of binary molecular compounds because they have similar formulas. Binary molecular compounds are named using the greek prefixes. Do not allow other instances of Greek or similar prefixes to confuse use in naming some of the oxyanions. For example, Cr2O72- is named dichromate. This has nothing to do with the naming of binary molecular compounds. There are a few instances of oxyanions series for a non-metal with two - - possible anions (e.g. NO3 , NO2 ). Remember the higher number of oxygens name ends in –ate. Most oxyanions with just one type in their series (e.g. only one type with Carbon and Oxygen: CO32-) will end in “-ate.” Cl, Br, and I each all form four oxyanions with the pattern (XO4-, XO3-, XO2-, XO-) where X=halogen and names respectively (per____ate, ____ate, ____ite, and hypo____ite). Fill the halogen name (or shortened name in each blank. Recall oxyanions that are charged –2 and –3 form hydrogen-containing polyatomic ions as well (e.g. HPO42- hydrogen phosphate). Remember all common acids dissolve in water. The prefix “hydro” does not necessarily indicate that it is an acid. Hydro means that the acid does not contain the element oxygen. Oxoacids do not begin with the prefix “hydro.” Chemical Equations and Balancing Write and Balance 1. If the equation is not written out, first write the chemical equation using names for each substance involved (reactants products). 2. Rewrite the equation by translating each word into the correct symbol or formula, indicating the state or condition after each (s), (l), (g), or (aq). 3. Balance the equation: a. Count up the total number of each atom in all formulas on each side of the equation. b. Balance any unbalanced atom by placing the necessary whole-number coefficient in front of the appropriate symbol or formula. The coefficient applies to the entire formula. Never change the subscript of a formula! c. Often, step b will unbalance another atom. Repeat steps a & b until all atoms are balanced. d. The equation is balanced when there is the same number of atoms of a given type on each side of the equation. Equation Formulation Tips a. The “formula” of any uncombined element is its symbol (e.g. Copper is Cu), except for the diatomic elements (H2, N2, O2, F2, Cl2, Br2, I2). b. The state of any element is solid, except: a. Hg, Br2 are liquids b. H2, N2, O2, F2, Cl2 are gases (as well as with the noble gases) c. Ionic compounds are in the solid state, except that they are usually dissolved in water, thus are aqueous (aq). Balancing Tips a. A rule of thumb for the order of balancing atoms is: Balance metals first, then non-metals, then hydrogen, then oxygen. b. Use the principle of Least Common Multiple to balance atoms. c. An uncombined element in the equation is good to balance last. d. Polyatomic ions that are present on both sides of the equation can be counted as a whole unit for ease. This is especially useful for double replacement reactions. e. Remember to multiply coefficients & subscripts, when counting atoms, for example: 3Ca3(PO4)2 has a total of ___ calcium ___ phosphorus ___ oxygen atoms cpiersol –2015.10.13 Piersol 10-17-2012 All Reactions Double Replacement Oxidation-Reduction Precipitation Combination (Synthesis) Acid-Base Decomposition Reactions may have more than one classification, but the following are mutually exclusive: Double Replacement and Oxidation-Reduction Single Replacement Combustion Synthesis and Decomposition Other 2H2(g) + O2(g) 2H2O(g) HNO3(aq) + KOH(aq) KNO3(aq) + H2O(l) Pb(NO3)2(aq) + KI(aq) PbI2(s) + KNO3(aq) KClO3(s) KCl(s) + O2(g) C6H12O6(s) + 6O2(g) 6CO2(g) + 6H2O(g) 2H2O(g) 2H2(g) + O2(g) Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g) 2Zn(s) + O2(g) 2ZnO(s) 2H2(g) + O2(g) 2H2O(g) combination (synthesis) combustion oxidation-reduction HNO3(aq) + KOH(aq) KNO3(aq) + H2O(l) acid-base double-replacement Pb(NO3)2(aq) + KI(aq) PbI2(s) + KNO3(aq) precipitation double-replacement KClO3(s) KCl(s) + O2(g) decomposition oxidation-reduction C6H12O6(s) + 6O2(g) 6CO2(g) + 6H2O(g) oxidation-reduction combustion 2H2O(g) 2H2(g) + O2(g) decomposition oxidation-reduction Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g) single-replacement oxidation-reduction 2Zn(s) + O2(g) 2ZnO(s) oxidation-reduction combination (synthesis) combustion Empirical Formula Determination (in 4 or 5 easy steps) 1. If given percent composition, take each percentage in grams (as if using a 100-gram sample). 2. Convert each element from grams à moles 3. Divide each element by the smallest number. 4. If the numbers are reasonably whole numbers, round each and use as subscripts. Otherwise, go to then next step. 5. Determine which decimal ending is close to that in the table below and multiply each by the common denominator. Principle of Common Denominator decimal (approximate) Multiply each by denominator: ending fraction 0.25 1/4 4 0.33 1/3 3 0.50 1/2 2 0.67 2/3 3 0.75 3/4 4 Stoichiometry Chart molar mass mole ratio Moles A Grams A A molar mass Grams B Moles B (equation) B PV=nRT n = PV RT Gas A Gas B • “A” represents the known quantity of substance A, which can be a reactant or product. • “B” represents an unknown quantity of substance B, which can be a reactant or product. Chemistry P106 Final Fact Sheet Important Stuff: Bring a pencil. Bring a scientific calculator. Bring a card no larger than 3”x5” filled with any desired information Bring a green scantron sheet with your name written on it. Use the restroom before you begin taking the final exam. Turn your cell phone off before you begin taking the final exam. Review 8 – 9:40 a.m. Thursday, July 21 Final Exam 10 a.m. – 12:15 p.m. Thursday, July 21 Majority of Topics Covered on the Final Exam: Chapter 1 – Introduction to Chemistry Terminology Scientific Method Physical and chemical change Physical and chemical properties Chapter 2 - Measurement Metric System Conversions Significant Digits (Figures) Temperature Conversions Density Just the facts, ma’am! Chapter 3 – Matter Classify matter: Elements, compounds, substances, homogeneous or heterogeneous mixtures Physical vs Chemical Change/Properties Chapter 4 – Elements, Atoms, Ions The 3 subatomic particles and their properties (mass, charge) Atomic number (= number of protons) Isotopes (same atomic number, different numbers of neutrons) Periodic Table classification (alkali metal, alkaline earth metals, etc) Chapter 5 – Nomenclature Responsible for naming compounds that contain the following anions: sulfate, sulfite, nitrate, nitrite, chlorate, chlorite, and halides (e.g. bromide) Name binary molecular (2 non-metals; uses Greek prefixes) Chapter 6 & 7 – Chemical Equations Principles, descriptors, coefficients Balancing equations Determine reaction type: combustion, double replacement (precipitation or acid/base), combination (synthesis), decomposition, redox Chapter 8 – Chemical Composition Avogadro’s number : 6.022 X 1023 = 1 mole Convert between any of the following: grams, moles, atoms, molecules Molar mass Percent composition Empirical formula calc Chapter 9 – Chemical Reaction Quantities (Stoichiometry) Convert moles A Moles B Convert grams A Moles B Convert grams A grams B Theoretical yield vs. actual yield Limiting Reactant Chapter 11 – Modern Atomic Theory Orbitals defined Electronic configuration of the elements Valence electrons Periodic Table – Classification by electron config / valence electrons Trends: atomic radius, ionization energy Chapter 12 – Chemical Bonding Covalent vs. ionic bonding (electronegativity trend) Draw Lewis structures: polyatomic ions, molecules Single, double, triple bonds Unpaired (non-bonding) electrons 3D Structures (VSEPR theory—geometries, bond angles, sketch structure) Bond and molecular polarity Chapter 13 – Gases Gas Laws: Boyle’s Law (P1V1 = P2V2) Charles’ Law (V1/T1 = V2/T2) Avogadro’s Law (V1/n1 = V2/n2) Ideal Gas Law: PV = nRT Dalton’s Law of Partial Pressures: Ptot = P1 + P2 + P3 + … Gas Stoichiometry Chapter 14 – Solids, Liquids Heating/Cooling curve (sketch & label) Intramolecular vs intermolecular forces Intermolecular forces: (DD, HB, LD), and predict properties trends Vapor Pressure Types of solids (Ionic, Molecular, Atomic) Chapter 15 – Solutions Solution = solute + solvent (definitions) Calculate mass percent solution Calculate molarity from (grams or moles) solute, and volume solution Calculate moles from molarity and volume, and convert to grams if needed. Also, know what each of these scientists contributed to chemistry: Dalton, J.J. Thomson, Mendeleev, Rutherford, Bohr, Schrödinger The Final Exam is worth 20% of your grade. Don’t forget to study!